Answer:
- <em>c. The reaction is spontaneous at all temperatures.</em>
Explanation:
The spontaneity of a reaction can be determined by the thermodynamic property named Gibb's free energy or simply free energy (G).
The change in the free energy of a system is defined as the difference between the increase in enthalpy (ΔH) and the product of the temperature (T) times the increase in entropy (ΔS):
The sign of ΔG tells if a reaction is spontaneous according to this:
- ΔG < 0, the reaction is spontaneous.
- ΔG = 0, the reaction is in equilibrium.
- ΔG > 0, the reaction is not spontaneous.
The question states that a reaction is exothermic, and its entropy change is positive. That means:
- Exhotermic: ΔH < 0
- Positive entropy change: ΔS > 0
Remember that the temperature is stated in absolute scale, so T is always positive.
Hence, ΔG = ΔH - T ΔS = (negative) - T (positive) = (negative) + (negative) = negative.
<u>Conclusion</u>: since ΔG is negative, regardless the temperature, you conclude that<em><u> the reaction is spontaneous at all temperatures, which is the option c.</u></em>
Hello,
The answer is option A "<span>the heat from the stove".
Reason:
The answer is option A because the variable the heat from the stove is causing the ice to change into water. Its not option B because thats not in the procedures. Its not option C because it is not a variable. Its also not D because thats also not a variable.
If you need anymore help feel free to ask me!
Hope this helps!
~Nonportrit</span>
As you move across a period, the atomic radii decreases. ... As you move across a period, electrons are added to the same energy level while protons are also being added. The concentration of more protons creates a higher effective nuclear charge.
